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How many moes of diethylamine((C2H5)2NH, Kb-1.3E-3) must be added to 447ml of distilled water to produce a solution with a pH of 12.787?
Can someone explain this step by step?
How many moles of sulfate ions (SO2-/4) are present in 1.6 moles Al2(SO4)3
Compounds containing carbon-carbon triple bond undergo the Diels-Alder reaction. Formulate the product formed by the reaction of
The compound X2Y is only partially dissociated in water solution to form X and Y2- ions. A 0.0100 m solution is found to freeze at -0.040°C. Calculate the apparent percent dissociation of X2Y. Kf for water = 1.86°C/m.
If iron(III) acetate is added to be 1 x 10^-10 M in a solution that is 0.10 M NH3, what is Qsp and will Fe(OH)3 precitate? the Ksp of Fe(OH)3 is 4x10^-38 and Kb for NH3 is 1.8x10^-5
The temperature of a block of copper metal (molar mass 63.55 g mol-1) fell by 8.52 K when the copper block released 64.5 J of heat. What is the mass of the copper block?
The total pressure in the system is found to be 3.0 atm and the mole fraction is 0.12. Find K(pressure) Can someone explain all the steps to get to the answer?
Maleic acid is a carbon-hydrogen-oxygen compound used in dyeing and finishing fabrics and as a preservative of oils and fats. In a combustion analysis, a 1.054- sample of maleic acid yields 1.599 of and 0.327 of.
Aqueous solutions of phosphoric acid and sodium nitrite are combined, and the following equilibrium is established. H3PO4 (aq) + NO2- (aq) = H2PO4-(aq) + HNO2 (aq). The equilibrium constant Kc for this reaction is greater than one. Based on this i..
What is the pH of this solution? What is the concentration of the molecular species H3PO4?
Estimate change in free energy for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous
What is the nickel ion concentration in a solution prepared by mixing 451 mL of 0.414 M nickel nitrate with 465 mL of 0.364 M sodium hydroxide?
Assuming that the total pressure of the gases is 1.52 and that their mole ratio is 94 : 4.0 : 1.5 : 0.50, calculate the partial pressure (in atmospheres) of each gas.
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